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Electrochemistry Essentials: Energy Interchange & Electrochemical Cells

Explore the fascinating world of electrochemistry, where chemical and electrical energy interact. Learn about oxidation (OIL) and reduction (RIG), and how batteries and plating processes work. Discover how electrochemical cells generate electricity from chemical reactions or drive reactions with electrical energy. Unravel the workings of voltaic and electrolytic cells, and delve into the components of voltaic cells like the anode, cathode, and salt bridge. Witness electron and ion flows, and grasp concepts like electrolysis and electroplating. Uncover how electricity can be produced from spontaneous redox reactions. Dive into the realm of electrolytic cells, where non-spontaneous redox reactions are induced by electricity, and explore processes like electroplating.

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Electrochemistry Essentials: Energy Interchange & Electrochemical Cells

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  1. Electrochemistry: The study of the interchange of chemical and electrical energy Oxidationis the loss of electrons (Increase in charge). OIL Reductionis the gain of electrons (Decrease in charge) RIG Electro-chemistry: Batteries and plating

  2. Can you make electricity with chemicals? You need: 2 metals and 2 solutions of the same metal (ions) The more active metal will LOSE electrons to the less active metal (it’s ions) which will GAIN Electrons

  3. Electrochemical Cells: Device capable of either generating electrical energy from chemical reactions or facilitating chemical reactions through the introduction of electrical energy • Voltaic Cells: • Produces electrical current • spontaneous chemical reactions •  ex. Battery • 2. Electrolytic Cells • Consumes electrical current • non-spontaneous and require electricity or battery •  ex. Electrolysis, electroplating

  4. Parts of the voltaic cell… Anode  the electrode where oxidation occurs After a period of time, the anode may appear to become smaller as it falls into solution. Cathode  the electrode where reduction occurs After a period of time it may appear larger, due to ions from solution plating onto it. Salt Bridge  a device used to maintain electrical neutrality in a voltaic cell. This may be filled with a salt solution. Electron Flow  always from anode to cathode (through the wire) Ion Flow  always through the salt bridge

  5. Cathode Anode

  6. VOLTAIC CELLS (also called electrochemical cells) 2 or more cells = a battery Electricitycan be made from a spontaneous redox reaction, instead of heat, light ... measured in volts 2 half cells 1 side loses electrons to the other side that gains The more active metal looses, higher on Chart J Cu+2 + 2e- Cu0 Zn0 Zn+2 + 2e- - ions flow in salt bridge e-’s flows on wire GER LEO anode cathode Copper metal Zinc metal Cu solution like CuSO4(aq) Zn solution like ZnSO4 (aq) “ Dead” battery has reached equilibrium, volts = 0

  7. ELECTROLYTIC CELLS Redox reactions that are not spontaneous andrequire electricity Electrolysis: splitting a chemical apart into its elements using electricity H2O  H2 (g) + O2 (g) + + battery H + + 1 e- H 0 H2O GER (cathode) O-2O 0 + 2e- LEO (anode)

  8. Also an Electrolytic cell (Requires electricity or a battery) Electroplating: adding a layer of a metal onto another metal (usually expensive metals onto cheaper metal) - + battery - fork to be plated - solution with metal ions - - metal for plating Ag+ Ag Ag+ + 1e- Ag0 Ag0 Ag+1 + 1 e- reduction oxidation anode cathode

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